According to the Arrhenius equation, in a graph of $\log k$ versus $\frac{1}{T}$, the slope will be . . . . . . .

The activation energy of a reaction is zero. The rate constant of this reaction

According to Arrhenius theory,the activation energy is

For a certain gaseous reaction,the temperature is increased by $10\,^{\circ}C$ from $25\,^{\circ}C$ to $35\,^{\circ}C$. If the rate of the reaction doubles,what will be the value of the activation energy $(E_a)$?

Which of the following plots gives the value of activation energy?

The rate of a reaction quadruples when the temperature changes from $293 \ K$ to $313 \ K$. Calculate the energy of activation of the reaction assuming that it does not change with temperature.